Question 1

Write the formula for the conjugate acid of HPO42-

Accepted Answer

Question 2

If the pH of seawater is 8.0, what is the hydroxide ion concentration in seawater?

Accepted Answer

The answer of If the pH of seawater is 8.0,...

Question 3

Calculate the pH of a solution containing 0.20 g of NaOH in 2,000.mL of solution.

Accepted Answer

The answer of Calculate the pH of a solution containing...

Question 4

What is the pH of a 0.0055 M HA (weak acid)solution that is 8.2% ionized?

Accepted Answer

A) 2.26 
B) 3.35 
C) 4.52 
D) 8.21 
E) 10.65 
A) 2.26 
B) 3.35 
C) 4.52 
D) 8.21 
E) 10.65

Question 5

Kw = 1.0 x 10-14 at all temperatures

Accepted Answer

A) True 
 B)False

Question 6

Write the chemical formula for the acid formed when Cl2O7 is dissolved in water.

Accepted Answer

Question 7

If the pH of tomato juice is 4.0, what is the hydroxide ion concentration in this solution?

Accepted Answer

The answer of If the pH of tomato juice is...

Question 8

Identify the conjugate acid of HCO3-

Accepted Answer

A) H2O 
B) CO32- 
C) H2CO3 
D) CO2 
E) H3O+ 
A) H2O 
B) CO32- 
C) H2CO3 
D) CO2 
E) H3O+

Question 9

In aqueous solutions at 25°C, the sum of the ion concentrations ([H+] + [OH -])equals 1 × 10 - 14.

Accepted Answer

A) True 
 B)False

Question 10

What mass of potassium hypochlorite must be added to 450.mL of water to give a solution with pH = 10.20? [Ka(HClO)= 4.0 × 10-8]

Accepted Answer

A) 20.g 
B) 0.032 g 
C) 4.1 g 
D) 2.4 g 
E) 9.1 g 
A) 20.g 
B) 0.032 g 
C) 4.1 g 
D) 2.4 g 
E) 9.1 g

Question 11

Predict the direction in which the equilibrium will lie for the reaction H2SO3(aq)+ HCO3- (aq)    
HSO3-(aq)+ H2CO3(aq).
Ka1(H2SO3)= 1 × 10-2; Ka1(H2CO3)= 4.2 × 10-7

Accepted Answer

A) to the right 
B) to the left 
C) in the middle 
A) to the right 
B) to the left 
C) in the middle

Question 12

In the reaction: CH3COOH(aq)+ NH2- (aq)      CH3COO- (aq)+ NH3(aq), the conjugate acid-base pairs are:

Accepted Answer

A) pair 1: CH3COOH and CH3COO- ; pair 2: NH2-  and NH3 
B) pair 1: CH3COOH and NH3; pair 2: NH2-  and CH3COO- 
C) pair 1: CH3COOH and NH2- ; pair 2: NH3 and CH3OO- 
D) pair 1: CH3COOH and CH3COO- ; pair 2: NH4+  and NH3 
E) pair 1: CH3COOH and CH3COO- ; pair 2: NH2-  and NH3+ 
A) pair 1: CH3COOH and CH3COO- ; pair 2: NH2-  and NH3 
B) pair 1: CH3COOH and NH3; pair 2: NH2-  and CH3COO- 
C) pair 1: CH3COOH and NH2- ; pair 2: NH3 and CH3OO- 
D) pair 1: CH3COOH and CH3COO- ; pair 2: NH4+  and NH3 
E) pair 1: CH3COOH and CH3COO- ; pair 2: NH2-  and NH3+

Question 13

What is the pH of a 0.080 M solution of the weak base pyridine (C5H5N; Kb = 1.7 x 10-9)

Accepted Answer

A) 8.77 
B) 5.23 
C) 4.93 
D) 12.90 
E) 9.07 
A) 8.77 
B) 5.23 
C) 4.93 
D) 12.90 
E) 9.07

Question 14

What mass of sodium formate (HCOONa)must be added to 350.mL of water in order to obtain a solution having a pH of 8.50? [Ka(HCOOH)= 1.77 × 10-4]

Accepted Answer

A) 0.23 g 
B) 4.3 g 
C) 35 g 
D) 12 g 
E) 130 g 
A) 0.23 g 
B) 4.3 g 
C) 35 g 
D) 12 g 
E) 130 g

Question 15

Aspartic acid (C4H7NO4), one of the 20 essential amino acids, has two ionizable hydrogens.At 25°C, Ka1 = 1.38 × 10-4 and Ka2 = 1.51 × 10-10.What is the concentration of doubly ionized aspartate ions in a 0.125 M aqueous solution of aspartic acid?

Accepted Answer

A) 3.33 × 10-2 M 
B) 4.16 × 10-3 M 
C) 4.15 × 10-3 M 
D) 1.51 × 10-10 M 
E) 2.08 × 10-14 M 
A) 3.33 × 10-2 M 
B) 4.16 × 10-3 M 
C) 4.15 × 10-3 M 
D) 1.51 × 10-10 M 
E) 2.08 × 10-14 M

Question 16

Which of these acids is stronger, H3AsO3 or H3AsO4?

Accepted Answer

Question 17

A 0.10 M HF solution is 8.4% ionized.Calculate the H+ ion concentration.

Accepted Answer

A) 0.84 M 
B) 0.12 M 
C) 0.10 M 
D) 0.084 M 
E) 8.4 × 10-3 M 
A) 0.84 M 
B) 0.12 M 
C) 0.10 M 
D) 0.084 M 
E) 8.4 × 10-3 M

Question 18

Which one of the following equations represents the ionization of a weak monoprotic acid in water?

Accepted Answer

A) HNO2(aq)+ OH- (aq)     H2O(l)+ NO2-(aq) 
B) HNO2(aq)+ NH3(aq)     NH4NO2(aq) 
C) HNO2(aq)+ H2O(l)     H3O+(aq)+ NO2-(aq) 
D) HNO3(aq)+ OH-(aq)     H2O(l)+ NO3-(aq) 
E) NO2- (aq)+ H2O(aq)     HNO2(aq)+ OH-(aq) 
A) HNO2(aq)+ OH- (aq)     H2O(l)+ NO2-(aq) 
B) HNO2(aq)+ NH3(aq)     NH4NO2(aq) 
C) HNO2(aq)+ H2O(l)     H3O+(aq)+ NO2-(aq) 
D) HNO3(aq)+ OH-(aq)     H2O(l)+ NO3-(aq) 
E) NO2- (aq)+ H2O(aq)     HNO2(aq)+ OH-(aq)

Question 19

Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized.

Accepted Answer

A) 1.00 
B) 0.00070 
C) 3.15 
D) 5.15 
E) 7.00 
A) 1.00 
B) 0.00070 
C) 3.15 
D) 5.15 
E) 7.00

Question 20

Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

Accepted Answer

A) 2.9 × 10-2 M 
B) 5.7 × 10-2 M 
C) 1.3 × 10-3 M 
D) 2.9 × 10-3 M 
E) 5.7 × 10-4 M 
A) 2.9 × 10-2 M 
B) 5.7 × 10-2 M 
C) 1.3 × 10-3 M 
D) 2.9 × 10-3 M 
E) 5.7 × 10-4 M

Exam 15: Acids and Bases

Write the formula for the conjugate acid of HPO42-

If the pH of seawater is 8.0, what is the hydroxide ion concentration in seawater?

Calculate the pH of a solution containing 0.20 g of NaOH in 2,000.mL of solution.

What is the pH of a 0.0055 M HA (weak acid)solution that is 8.2% ionized?

Kw = 1.0 x 10-14 at all temperatures

Write the chemical formula for the acid formed when Cl2O7 is dissolved in water.

If the pH of tomato juice is 4.0, what is the hydroxide ion concentration in this solution?

Identify the conjugate acid of HCO3-

In aqueous solutions at 25°C, the sum of the ion concentrations ([H+] + [OH -])equals 1 × 10 - 14.

What mass of potassium hypochlorite must be added to 450.mL of water to give a solution with pH = 10.20? [Ka(HClO)= 4.0 × 10-8]

Predict the direction in which the equilibrium will lie for the reaction H2SO3(aq)+ HCO3- (aq) HSO3-(aq)+ H2CO3(aq). Ka1(H2SO3)= 1 × 10-2; Ka1(H2CO3)= 4.2 × 10-7

In the reaction: CH3COOH(aq)+ NH2- (aq) CH3COO- (aq)+ NH3(aq), the conjugate acid-base pairs are:

What is the pH of a 0.080 M solution of the weak base pyridine (C5H5N; Kb = 1.7 x 10-9)

What mass of sodium formate (HCOONa)must be added to 350.mL of water in order to obtain a solution having a pH of 8.50? [Ka(HCOOH)= 1.77 × 10-4]

Aspartic acid (C4H7NO4), one of the 20 essential amino acids, has two ionizable hydrogens.At 25°C, Ka1 = 1.38 × 10-4 and Ka2 = 1.51 × 10-10.What is the concentration of doubly ionized aspartate ions in a 0.125 M aqueous solution of aspartic acid?

Which of these acids is stronger, H3AsO3 or H3AsO4?

A 0.10 M HF solution is 8.4% ionized.Calculate the H+ ion concentration.

Which one of the following equations represents the ionization of a weak monoprotic acid in water?

Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized.

Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

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Write the formula for the conjugate acid of HPO₄^2-

K_w = 1.0 x 10^-14 at all temperatures

Write the chemical formula for the acid formed when Cl₂O₇ is dissolved in water.

Identify the conjugate acid of HCO₃^-

In aqueous solutions at 25°C, the sum of the ion concentrations ([H⁺] + [OH^-])equals 1 × 10^{- 14}.

What mass of potassium hypochlorite must be added to 450.mL of water to give a solution with pH = 10.20? [K_a(HClO)= 4.0 × 10^-8]

Predict the direction in which the equilibrium will lie for the reaction H₂SO₃(aq)+ HCO₃^-(aq) HSO₃^-(aq)+ H₂CO₃(aq). K_a1(H₂SO₃)= 1 × 10^-2; K_a1(H₂CO₃)= 4.2 × 10^-7

In the reaction: CH₃COOH(aq)+ NH₂^- (aq) CH₃COO^- (aq)+ NH₃(aq), the conjugate acid-base pairs are:

What is the pH of a 0.080 M solution of the weak base pyridine (C₅H₅N; K_b = 1.7 x 10^-9)

What mass of sodium formate (HCOONa)must be added to 350.mL of water in order to obtain a solution having a pH of 8.50? [K_a(HCOOH)= 1.77 × 10^-4]

Aspartic acid (C₄H₇NO₄), one of the 20 essential amino acids, has two ionizable hydrogens.At 25°C, K_a1 = 1.38 × 10^-4 and K_a2 = 1.51 × 10^-10.What is the concentration of doubly ionized aspartate ions in a 0.125 M aqueous solution of aspartic acid?

Which of these acids is stronger, H₃AsO₃ or H₃AsO₄?

A 0.10 M HF solution is 8.4% ionized.Calculate the H⁺ ion concentration.